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A zinc electrode is submerged in an acidic 0.80M Zn+ solution which are connected by salt bridge to a 1.30M Ag+ solution containing a silver electrode. Determine the initial voltage of the cell at 298k
Given that:
Zn/Zn2+ E°=0.76V
Ag+/Ag E°=0.80V
Given the Ag+/Ag=0.8V, Cu2+/Cu=0.34V Calculate the standard emf of the cell and the equilibrium constant
Given Cu2+/Cu=0.34V and Cu2+/Cu+=0.153V, calculate the equilibrium constant for the reaction Cu + Cu2+<->2Cu2+
Calculate the emf of the following voltaic cells;
(a) Pt/Fe2+(0.1M),Fe3+(0.2M)//Ag+(1M)/Ag
(b)Zn/Zn3+(10^-3M)//Ag+(10^-3M)/Ag
(c)Al/Al3+(0.1M)//Sn2+(0.37M)/Sn
Given Fe3+/Fe2+=0.77V, Zn2+/Zn=-0.76V, Sn2+/Sn=-0.14V, Ag+/Ag=0.8V, Al3+/Al=-2.56V
Calculate the emf of the following voltaic cells;
(a) Pt/Fe2+(0.1M),Fe3+(0.2M)//Ag+(1M)/Ag
(b)Zn/Zn3+(10^-3M)//Ag+(10^-3M)/Ag
(c)Al/Al3+(0.1M)//Sn2+(0.37M)/Sn
Given that Zn/Zn2+(1M)//Cu2+(1M)/Cu
(a) calculate the emf of the cell
(b) predict if the reaction is spontaneous or non spontaneous
Given that Zn/Zn2+ E=0.34V, Cu2+/Cu E=1.10V
Given that Zn/Zn+ E=-0.76V and cu+/Cu E=+0.33V (a) calculate the end of the cell (b) predict it's spontaneous or non spontaneous
What will be the molecular Hamiltonian for BeH2 molecule?
Addition reaction of carbonyl compounds
Water H2o
The arithmetic signs of qrev denote the loss heat by the of system and the gain of heat by the surrounding. since Tsys > Tsun in this case the the entropy change for the surroundings will be greater than that will give a por so the sum ASsys and ASsun OF positive value For ∆SunivThe arithmetic signs of qrev denote the loss heat by the of system and the gain of heat by the surrounding. since Tsys > Tsun in this case the the entropy change for the surroundings will be greater than that will give a por so the sum ASsys and ASsun OF positive value For ∆Suniv
